22. K, = 1.8 x 10s for acetic acid (HC2H3O2) Part 1. What molar ratio of acetic acid to sodium acetate ([acetic acid]/[sodium acetate]) is required to create a buffer solution having a pH of 4.89 at 25 C? a) 0.56 b) 1.4 c) 0.71 d) 2.0 e) 2.9 f) none of the above Part 2. Which of the following processes will decrease the pH of the above buffer solution (Part 1) from 4.89 to 4.50. a) Adding more sodium acetate b) Adding more water c) Adding some NH&CI d) none of the above

22. K, = 1.8 x 10s for acetic acid (HC2H3O2) Part 1. What molar ratio of acetic acid to sodium acetate ([acetic acid]/[sodium acetate]) is required to create a buffer solution having a pH of 4.89 at 25 C? a) 0.56 b) 1.4 c) 0.71 d) 2.0 e) 2.9 f) none of the above Part 2. Which of the following processes will decrease the pH of the above buffer solution (Part 1) from 4.89 to 4.50. a) Adding more sodium acetate b) Adding more water c) Adding some NH&CI d) none of the above

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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I just need assistance with part B 5a) Calculate the pH of a buffer solution that contains 0.79 M NaH2PO4 and 0.13M Na2HPO4 Answer: 6.43 5b) Calculate the change in pH if 0.050 g of solid NaOH is added to 150 mL of the solution in the problem above.
0.05 mole of HCI is added to one liter of buffer containing 0.04 mole of NH,OH and 0.03 mole of NH,CI. What is the pH? (you can subtract add moles but not molarity)Kb = 1.8 X 10*
Please don't provide handwritten solution... A 1.0 L solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value for Ka HC2H3O2 is 1.8 X 10-5. What is the pH of the buffer after adding 0.010 mol NaOH to the buffer.
3. A buffer solution contains 0.125 moles of ammonium chloride added to 500.0 ml of 0.500 M solution of ammonia. A) What is the pH of this buffer? B) What is the pH after the addition of 0.0100 moles of HCI bubbled into 500.0 mL of the buffer?
18) What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains 0.25 mole HF and 0.15 mole NaF? (K, = 6.8 x 10* for HF)
Dino needs to prepare 200.0 mLs of a 0.25M /0.20 M buffer solution that has pH of 4.7. To make this buffer solution, Dino has available 0.50 M solutions each of the following: Chemicals .. NH3/NH4CI •HCOOH/HCOOK HONH2/HONH3CI CH3COOH/NaCH3COO ● NH3/NH4CI HONH2/HONH3C HCOOH/HCOOK K₂ Which set of conjugate acid - base pairings should Dino select? CH3COOH/NaCH3COO 1.78 x 10-5 5.62 x 10-10 1.82 x 10-4 9.12 x 10-9
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es) 1. Calculate the volume of the salt to be used in the preparation of 200 ml of the following buffer solutions. BUFFER DESIRED NUMBER pH 1 2 3 4 7.18 9.45 8.25 6.90 0.1M SOLUTIONS NaH2PO4/Na2HPO4 NH4CI/NH3 NH4CI/NH3 NaH2PO4/Na2HPO4 pka wwwwww 6.80 9.30 9.30 6.80 VOLUME OF ACID (ml) VOLUME OF SALT (ml)